Upload
jaguilar
View
1.507
Download
1
Tags:
Embed Size (px)
DESCRIPTION
The Chemistry of Life
Citation preview
Ch 6: The Chemistry of LifeCh 6: The Chemistry of Life
6.1 - Atoms and Their Interactions
6.1 - Atoms and Their Interactions
Section 6.1Section 6.1
What is an Element?
What are Atoms?
2 Types of Chemical Bonds
Chemical Reactions
Inside This Section...Inside This Section...
A substance that can not be broken down into smaller particles.
90 elements naturally occur on earth
25 are essential to living things
Each element is identified by a symbol
What is an Element?What is an Element?
Section 6.1Section 6.1
ElementsElements
Section 6.1Section 6.1
C = CarbonCa = Calcium
Na = Sodium
ElementsElements
Section 6.1Section 6.1
K = Potassium
N = Nitrogen
Fe = Iron
ElementsElements
Section 6.1Section 6.1
AU = Gold
Elements that are present in small amounts in the human body.
N,K,Ca, and Fe are a few examples
Help control cell metabolism
Plants obtain trace elements through their roots while animals obtain trace elements through what they eat.
Trace ElementsTrace Elements
Section 6.1Section 6.1
The smallest part of an element that still maintains all the characteristics of that element.
The basic building blocks of all matter
What is an Atom?What is an Atom?
Section 6.1Section 6.1
Nucleus: Center of the Atom
Electrons:
The outer particles
Negatively charged
Protons:
Particles found in the nucleus
Positively charged
Neutrons: Particles found in the nucleus that have no charge.
What is an Atom?What is an Atom?
Section 6.1Section 6.1
What is an Atom?What is an Atom?
Section 6.1Section 6.1
Electron (-)
Proton (+)
Neutron (0)
Electron and Proton numbers are always the same
Energy LevelsEnergy Levels
Section 6.1Section 6.1
Regions around the nucleus that the electrons travel.Atoms like to have their outer most energy level full.
Energy Levels & ElectronsEnergy Levels & Electrons
Section 6.1Section 6.1
Energy LevelEnergy Level # of # of ElectronsElectrons
1 2
2 8
3 18
Atoms of the same element that have different numbers of neutrons.
What are Isotopes?What are Isotopes?
Section 6.1Section 6.1
Most carbon nuclei contain six neutrons
Some have 7 or 8
These three atoms are isotopes
We refer to the isotopes in terms of the combined total of protons and neutrons
Carbon-12 has 6 protons and 6 neutrons
How many protons and neutrons does carbon-13 and carbon-14 have??
What are Isotopes?What are Isotopes?
Section 6.1Section 6.1
Read Problem Solving Lab 6.1 in groups of twos (pg 149)
Answer the 4 questions
Problem Solving Lab 6.1Problem Solving Lab 6.1
Section 6.1Section 6.1
A substance that is composed of two or more different elements that are chemically combined.
Properties of compounds are different than those of their individual elements. (NaCl)
Compounds can always be described with an equation. (H20)
CompoundsCompounds
Section 6.1Section 6.1
When two elements share electrons in their outer energy level.
Atoms are the happiest when their outer energy level is full.
Water is an example
Bond #1: Covalent BondsBond #1: Covalent Bonds
Section 6.1Section 6.1
A bond between atoms that is formed by losing and gaining an electron.
NaCl is an example
Na has one electron in its outer shell
Cl has 7 in its outer shell
The two oppositely charged atoms now attract each other like magnets.
Bond #2: Ionic BondBond #2: Ionic Bond
Section 6.1Section 6.1
Chemical reactions occur when bonds between compounds are broken or formed.
Chemical reactions must have the right environment
pH
Temperature
Energy
Concentration
Chemical ReactionsChemical Reactions
Section 6.1Section 6.1
Reactant + reactant --> Product
Reactants undergo chemical reactions
Products are formed in chemical reactions
2H2 + O2 --> 2H2O
Key Point: atoms are never created or destroyed
Chemical EquationsChemical Equations
Section 6.1Section 6.1
All of the chemical reactions that occur in the human body.
Produce energy
Require energy
Build necessary molecules for bodily functions
MetabolismMetabolism
Section 6.1Section 6.1
Solution: A mixture in which one or more substances are evenly distributed in another substance.
Salt Water
Kool-Aid
Solutions and MixturesSolutions and Mixtures
Section 6.1Section 6.1
Mixture: A combination of substances in which the individual components retain their chemical properties.Sand and Salt
pH is a measure of how acidic or basic a substance is.
Scale of 0-14
pH paper is used to determine the pH level
A pH below 7 is acidic
A pH above 7 is basic
A pH of 7 is neutral (Water)
pH LevelspH Levels
Section 6.1Section 6.1
pH LevelspH Levels
Section 6.1Section 6.1
Any substance that forms hydrogen ions in water.
H+
When HCl is put into water H+ and Cl- ions.
AcidAcid
Section 6.1Section 6.1
Any substance that forms hydroxide ions in water.
OH-
When NaOH is put in water you get Na+ and OH- ions.
BaseBase
Section 6.1Section 6.1
Acids
Orange Juice
Stomach Acids
Tomato Juice
Common Acids and BasesCommon Acids and Bases
Section 6.1Section 6.1
Bases
Toothpaste
Baking Powder
Chlorine Bleach
Section 6.1Section 6.1
What is an Element?
What are Atoms?
2 Types of Chemical Bonds
Chemical Reactions
In Review...In Review...
Section 6.2Section 6.2
What are some characteristics of water?
How do organisms use water to live and grow?
Jump StartJump Start
Ch 6: The Chemistry of LifeCh 6: The Chemistry of Life
6.2 - Water and Diffusion
6.2 - Water and Diffusion
Section 6.2Section 6.2
The Importance of Water
The Characteristics of Water
Bond #3: Hydrogen Bonds
Diffusion
Inside This Section...Inside This Section...
Most life processes occur only in water
Helps to transport materials in organism
70 to 95% of most organisms is Water
The Importance of WaterThe Importance of Water
Section 6.2Section 6.2
Water is polar
Water sticks but isn’t sticky
Capillary action: able to creep up thin tubes
Water resists temperature changes
Water expands when it freezes
The Characteristics of WaterThe Characteristics of Water
Section 6.2Section 6.2
Water (H2O) contains two hydrogen atoms and one Oxygen atom that are covalently bonded to each other
The Shared electrons are more attracted to the Oxygen atom than to the hydrogen atoms (Unequal sharing)
Results in a polar molecule: It has a positive and a negative end
Polar likes polar (i.e. Ionic compounds like salt and other polar molecules like sugar)
Water is PolarWater is Polar
Section 6.2Section 6.2
Because water molecules have a positive end and a negative end, there will be an attraction between water molecules
This results in Hydrogen Bonds between the oxygen atom of one molecule and the hydrogen atom of another
Weaker Bond
Bond #3: Hydrogen BondsBond #3: Hydrogen Bonds
Section 6.2Section 6.2
It takes a lot of energy to increase its temperature
Loses a lot of heat when it cools
These features help maintain a steady environment (i.e. in cells)
What Resists Temperature ChangeWhat Resists Temperature Change
Section 6.2Section 6.2
Ice Floats - less dense
What would happen to lake Michigan if ice was more dense than water?
Water expands when it freezesWater expands when it freezes
Section 6.2Section 6.2
Anything that is moving has kinetic energy
If you look at the molecules of gasses, liquids and some solid molecules under a very powerful microscope, you will see that they are randomly moving --> Brownian motion
Brownian MotionBrownian Motion
Section 6.2Section 6.2
Diffusion: The net movement of particles from an area of higher concentration to an area of lower concentration.
A very slow process --> Relies on random molecular motion (Brownian motion)
Affected by 3 factors
Concentration (most important factor)
Temperature
Pressure
DiffusionDiffusion
Section 6.2Section 6.2
DiffusionDiffusion
Section 6.2Section 6.2
Diffusion continues until the two substances are distributed evenly --> Dynamic Equilibrium
Concentration gradient: the difference in concentration of a substance across space.
At dynamic equilibrium, there is no concentration gradient
DiffusionDiffusion
Section 6.2Section 6.2
Section 6.2Section 6.2
The Importance of Water
The Characteristics of Water
Bond #3: Hydrogen Bonds
Diffusion
In Review...In Review...
Ch 6: The Chemistry of LifeCh 6: The Chemistry of Life
6.3 - Life Substances6.3 - Life Substances
Section 6.3Section 6.3
The Structure of Carbon
Carbohydrates
Lipids
Proteins
Nucleic Acids
Inside This Section...Inside This Section...
Carbon has 4 electrons in its outer energy level
Can form 4 covalent bonds with other elements
Can also bond with other carbon atoms
CarbonCarbon
Section 6.3Section 6.3
CC
3 types of bonds:
Single bond: each atom shares 1 electron
Double bond: each atom shares 2 electrons
Triple bond: each atom shares 3 electrons
CarbonCarbon
Section 6.3Section 6.3
CC
CarbonCarbon
Section 6.3Section 6.3
CC CC
C C
CarbonCarbon
Section 6.3Section 6.3
CC CC
C C
Carbon atoms can form straight chains, branched chains, or rings and can bind to other elements
Can form a whole bunch of carbon structures
CarbonCarbon
Section 6.3Section 6.3
CC
Water - H2O
Glucose - C6H12O6
Isomers: Same simple formula but different 3D structure
Glucose and Galactose are both C6H12O6
Simple FormulasSimple Formulas
Section 6.3Section 6.3
Large molecules are called macromolecules (e.g. proteins)
Macromolecules are formed by binding together smaller molecules into chains (Polymer)
Molecular ChainsMolecular Chains
Section 6.3Section 6.3
Condensation: Chemical reaction by which polymers are formed (water is removed)
Hydrolysis: Chemical reaction by which polymers are broken apart (water is used)
Condensation and HydrolysisCondensation and Hydrolysis
Section 6.3Section 6.3
Organic compound composed of Carbon, hydrogen and oxygen.
2 H’s and 1 O for every carbon
Simplest type is monosaccharides like glucose and fructose.
CarbohydratesCarbohydrates
Section 6.3Section 6.3
Two monosaccharides bind to form a disaccharide (i.e. Sucrose = glucose + fructose)
Many monosaccharides bind to form polysaccharides (i.e. starch and cellulose - glucose polymers)
CarbohydratesCarbohydrates
Section 6.3Section 6.3
Section 6.3Section 6.3
monosaccharide (glucose)
disaccharide (sucrose)
polysaccharide (starch)
Lipids are fats and oils.
Organic compound with a large proportion of C-H bonds and less oxygen than carbohydrates.
Nonpolar
Used in cells for energy storage, insulation and protection.
LipidsLipids
Section 6.3Section 6.3
Most commonly 3 fatty acids bound to a glycerol molecule. (pg 164)
LipidsLipids
Section 6.3Section 6.3
Provide structure for tissues and organs
Carry out cell metabolism
Large, complex polymer made of Carbon, hydrogen, oxygen, nitrogen and usually sulfur.
Building blocks are various combinations of amino acids
Amino acids join together with peptide bond
ProteinsProteins
Section 6.3Section 6.3
An Enzyme is a protein that changes the rate of a chemical reaction
Involved in almost all metabolic processes.
Speed up chemical reactions
ProteinsProteins
Section 6.3Section 6.3
Stores cellular information in the form of a code.
Polymer of smaller subunits called nucleotides.
Nucleotides consist of C, H, O, N, P atoms.
Nucleotides make up our DNA
Nucleic AcidsNucleic Acids
Section 6.3Section 6.3
Nucleic acids have 3 parts:
A Base
A Simple sugar
A Phosphate group
Nucleic AcidsNucleic Acids
Section 6.3Section 6.3
NitrogenouNitrogenous Bases BasePhospPhosp
hatehateO
SugSugarar
O
Nucleic AcidsNucleic Acids
Section 6.3Section 6.3
NitrogenouNitrogenous Bases BasePhospPhosp
hatehateO
SugSugarar
O
Section 6.3Section 6.3
The Structure of Carbon
Carbohydrates
Lipids
Proteins
Nucleic Acids
In Review...In Review...